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Chapter 11: Problem 18

Write equations showing the ions present after the following strong electrolytes are dissolved in water. a. \(\mathrm{HNO}_{3}\) b. \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) c. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) d. \(\mathrm{SrBr}_{2}\) e. \(\mathrm{KClO}_{4}\) f. \(\mathrm{NH}_{4} \mathrm{Br}\) g. \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) h. \(\mathrm{CuSO}_{4}\) i. NaOH

Short Answer

Expert verified
a. \(\mathrm{HNO}_{3} \rightarrow \mathrm{H}^{+} + \mathrm{NO}_{3}^{-}\) b. \(\mathrm{Na}_{2} \mathrm{SO}_{4} \rightarrow 2\mathrm{Na}^{+} + \mathrm{SO}_{4}^{2-}\) c. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3} \rightarrow \mathrm{Al}^{3+} + 3\mathrm{NO}_{3}^{-}\) d. \(\mathrm{SrBr}_{2} \rightarrow \mathrm{Sr}^{2+} + 2\mathrm{Br}^{-}\) e. \(\mathrm{KClO}_{4} \rightarrow \mathrm{K}^{+} + \mathrm{ClO}_{4}^{-}\) f. \(\mathrm{NH}_{4} \mathrm{Br} \rightarrow \mathrm{NH}_{4}^{+} + \mathrm{Br}^{-}\) g. \(\mathrm{NH}_{4} \mathrm{NO}_{3} \rightarrow \mathrm{NH}_{4}^{+} + \mathrm{NO}_{3}^{-}\) h. \(\mathrm{CuSO}_{4} \rightarrow \mathrm{Cu}^{2+} + \mathrm{SO}_{4}^{2-}\) i. \(\mathrm{NaOH} \rightarrow \mathrm{Na}^{+} + \mathrm{OH}^{-}\)

Step by step solution

01

a. Dissociation of \(\mathrm{HNO}_{3}\)#

When \(\mathrm{HNO}_{3}\) dissolves in water, it dissociates into hydrogen ions (\(\mathrm{H}^{+}\)) and nitrate ions (\(\mathrm{NO}_{3}^{-}\)). The equation for the dissociation of \(\mathrm{HNO}_{3}\) is: \(\mathrm{HNO}_{3} \rightarrow \mathrm{H}^{+} + \mathrm{NO}_{3}^{-}\)
02

b. Dissociation of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\)#

When \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) dissolves in water, it dissociates into two sodium ions (\(\mathrm{Na}^{+}\)) and a sulfate ion (\(\mathrm{SO}_{4}^{2-}\)). The equation for the dissociation of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) is: \(\mathrm{Na}_{2} \mathrm{SO}_{4} \rightarrow 2\mathrm{Na}^{+} + \mathrm{SO}_{4}^{2-}\)
03

c. Dissociation of \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\)#

When \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) dissolves in water, it dissociates into an aluminum ion (\(\mathrm{Al}^{3+}\)) and three nitrate ions (\(\mathrm{NO}_{3}^{-}\)). The equation for the dissociation of \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) is: \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3} \rightarrow \mathrm{Al}^{3+} + 3\mathrm{NO}_{3}^{-}\)
04

d. Dissociation of \(\mathrm{SrBr}_{2}\)#

When \(\mathrm{SrBr}_{2}\) dissolves in water, it dissociates into a strontium ion (\(\mathrm{Sr}^{2+}\)) and two bromide ions (\(\mathrm{Br}^{-}\)). The equation for the dissociation of \(\mathrm{SrBr}_{2}\) is: \(\mathrm{SrBr}_{2} \rightarrow \mathrm{Sr}^{2+} + 2\mathrm{Br}^{-}\)
05

e. Dissociation of \(\mathrm{KClO}_{4}\)#

When \(\mathrm{KClO}_{4}\) dissolves in water, it dissociates into a potassium ion (\(\mathrm{K}^{+}\)) and a perchlorate ion (\(\mathrm{ClO}_{4}^{-}\)). The equation for the dissociation of \(\mathrm{KClO}_{4}\) is: \(\mathrm{KClO}_{4} \rightarrow \mathrm{K}^{+} + \mathrm{ClO}_{4}^{-}\)
06

f. Dissociation of \(\mathrm{NH}_{4} \mathrm{Br}\)#

When \(\mathrm{NH}_{4} \mathrm{Br}\) dissolves in water, it dissociates into an ammonium ion (\(\mathrm{NH}_{4}^{+}\)) and a bromide ion (\(\mathrm{Br}^{-}\)). The equation for the dissociation of \(\mathrm{NH}_{4} \mathrm{Br}\) is: \(\mathrm{NH}_{4} \mathrm{Br} \rightarrow \mathrm{NH}_{4}^{+} + \mathrm{Br}^{-}\)
07

g. Dissociation of \(\mathrm{NH}_{4} \mathrm{NO}_{3}\)#

When \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) dissolves in water, it dissociates into an ammonium ion (\(\mathrm{NH}_{4}^{+}\)) and a nitrate ion (\(\mathrm{NO}_{3}^{-}\)). The equation for the dissociation of \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) is: \(\mathrm{NH}_{4} \mathrm{NO}_{3} \rightarrow \mathrm{NH}_{4}^{+} + \mathrm{NO}_{3}^{-}\)
08

h. Dissociation of \(\mathrm{CuSO}_{4}\)#

When \(\mathrm{CuSO}_{4}\) dissolves in water, it dissociates into a copper ion (\(\mathrm{Cu}^{2+}\)) and a sulfate ion (\(\mathrm{SO}_{4}^{2-}\)). The equation for the dissociation of \(\mathrm{CuSO}_{4}\) is: \(\mathrm{CuSO}_{4} \rightarrow \mathrm{Cu}^{2+} + \mathrm{SO}_{4}^{2-}\)
09

i. Dissociation of \(\mathrm{NaOH}\)#

When \(\mathrm{NaOH}\) dissolves in water, it dissociates into a sodium ion (\(\mathrm{Na}^{+}\)) and a hydroxide ion (\(\mathrm{OH}^{-}\)). The equation for the dissociation of \(\mathrm{NaOH}\) is: \(\mathrm{NaOH} \rightarrow \mathrm{Na}^{+} + \mathrm{OH}^{-}\)

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Most popular questions from this chapter

In a coffee-cup calorimeter, 1.60 \(\mathrm{g} \mathrm{NH}_{4} \mathrm{NO}_{3}\) was mixed with 75.0 \(\mathrm{g}\) water at an initial temperature \(25.00^{\circ} \mathrm{C}\) . After dissolution of the salt, the final temperature of the calorimeter contents was \(23.34^{\circ} \mathrm{C}\) . a. Assuming the solution has a heat capacity of 4.18 \(\mathrm{J} / \mathrm{g}\) \(^{\circ} \mathrm{C},\) and assuming no heat loss to the calorimeter, calculate the enthalpy of solution \(\left(\Delta H_{\mathrm{soln}}\right)\) for the dissolution of \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) in units of $\mathrm{kJ} / \mathrm{mol} .$ b. If the enthalpy of hydration for \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) is $-630 . \mathrm{kJ} / \mathrm{mol}\( calculate the lattice energy of \)\mathrm{NH}_{4} \mathrm{NO}_{3} .$

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